What is the pH of a saturated solution of Ca(OH)2 if the solubility of calcium hydroxide is 1.50 g/L?
Formula: Ca(OH)2 ⇌ Ca2+ + 2 OH¯
Solubility product is written as:
Ksp = [Ca2+] [OH¯]2
DATA: Solubility (s) = 1.50 g/L = 0.0202 M (Convert g/L into molarity by dividing g/L by molar mass of Ca(OH)2
This is an important point: what we have calculated is 's' and it is NOT the [OH¯] for the given compound Ca(OH)2. That value is '2s.'
Because: Ksp = [Ca2+] [OH¯]2 = [s] [2s]2
[OH¯] = 2s = 2 x 0.0202 M = 0.0404 M
pOH = - log (0.0404) = 1.393 [As POH = -log (OH-)]
pH = 14 - 1.393 = 12.606 [ As PH = 14 - POH ]
Final answer: pH of the saturated solution of Ca(OH)2 = 12.606
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